What is the total pressure of a gaseous mixture that contains three gases with partial pressures of 0.845 atm, 120 torr and 210 mm Hg?
A)1175 torr
B)972 torr
C)0.411 atm
D)331 torr

Question

Quizplus · Accepted Answer

To find the total pressure of a gaseous mixture, you add up the partial pressures of all the gases in the mixture. However, you must ensure all pressures are in the same units before adding them. The given pressures are in different units: atm, torr, and mm Hg. 1 atm = 760 torr, and 1 torr = 1 mm Hg. Therefore, convert the pressures into torr before adding: 0.845 atm * 760 torr/atm = 642 torr, 120 torr (already in torr), and 210 mm Hg = 210 torr (since 1 mm Hg = 1 torr). Adding these together gives 642 + 120 + 210 = 972 torr.

What Is the Total Pressure of a Gaseous Mixture That